1. Combination Reaction :Two or more reactant combine to form a single product. 2 Mg (s) + O2 (g) → 2 MgO Magnesium Oxygen Magnesium oxide (White ash) (basic) turns Red litmus blue 2. Decomposition Reaction: A single compound decomposes or break down to give two or moresimpler substances. 2 FeSO4 (s).symbol of het Fe2 O3 (s) + SO2 (g) + SO3(g) Ferrous Sulphate Ferric oxide SULPHUR Sulphur (green) (brown) dioxide trioxide 3. Displacement Reaction: A more reactive element [metal] displaces less reactive elemen [metal] from its aqueous salt soln Fe (s) + ZnSO4 (aq)      → FeSO4 (aq) + Zn (s) (Colourless) (green) 4. Double Displacement Reaction: Aqueous soln of two ionic compounds react by exchange of their ions is called double displacement Reaction BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2 NaCl (aq) Pb(NO3)2 + 2 KI (aq) → PBI2 ( ↓ ) + 2 KNO3 (aq) 5. Oxidation Reaction: In oxidation reaction, addition of oxygen or removal of hydrogen or loss of electron takes PLACE. 2 Mg(s) + O2 (g)  →  2MgO (s)  2 Cu + O2  →  2 CuO (Black ) (Copper II Oxide)   6. Reduction Reaction: In reduction Reaction addition of hydrogen or removal of oxygen or gain of electron takes place. CuO(s) + H2 (g)  →Cu(s) + H2 O (l)   7. Redox Reaction: Reaction involving both oxidation and reduction simultaneously CuO (s)+ H2   →  Cu(s) + H2 O (l).   8. EXOTHERMIC Reaction: Reaction in which heat is evolved. C (s) + O2 (g)   → CO2 (g) + Heat 10. Neutralisation Reaction : When an acid and a base react together to form salt and water.  HCl (aq)  +  NaOH (aq)  →  H2O (l)  +  NaCl (aq)  (acid) (base)  (Water) (Salt)  Hydrochloric acid  Sodium hydroxide   Sodium ChlorideExplanation: